Shells are made up of orbitals; orbitals can hold up to 2 electrons
Each shell can hold2n squared electrons
The number of orbitals increases with each new type of orbitals: s,1 p,3 d,5 f,7
two electrons fit into each orbital so the number of electrons also increases in each sub-shell:
s, 1x2=2 p,2x3=6 d, 2x5=10 f, 2x7=14
3d has a higherenergy level then 4s
With the box model fill in each box with on arrow first the repeat with alternate arrows
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Ionic Bonding and Structure
An ionic bond is an attraction between two oppositely charged ions
Ionic bonding is when one atom donates electrons to become a positive cation and the other atom recieves electrons to become a neagtive anion
Ionic compounds are structured in giant ionic lattices
Almost all ionic compounds are solids at room temp
Have high MP and BP due to the strong electrostatic forces of attraction between the ions
The larger the charges on the ions, the stronger the attraction, the higher the BP
The larger the size of the ion, the stronger the attraction
Ionic compounds dissolve in polar substances such as water. However with large charges, the attraction may be too strong for water to break down decreasing the solubility
Won't conduct as solids as ions are in fixed positions so there are no mobile charge carriers
Will conduct when molten or dissolved in water as ions are free to move so there are mobile charge carriers
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Covalent Bonding
Covalent bonding is the electrostatic attraction between a shared pair of electrons and the nuclie of the bonded atoms
Found in: diatomic molecules, non-metallic compounds, polyatomic compounds
A covelent bond is the overlap of two atomic orbitals
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